Answer: 2.17x10⁻³ atm
Explanation:
First, we must write the balanced chemical equation for the process:
C₂H₄(g) + H₂O(g) ⇌ C₂H₅OH(g)
The chemical reactions that occur in a closed container can reach a state of <u>chemical equilibrium</u> that is characterized because the concentrations of the reactants and products remain constant over time. The <u>equilibrium constant</u> of a chemical reaction is the value of its reaction quotient in chemical equilibrium.
The equilibrium constant (K) is expressed as <u>the ratio between the molar concentrations (mol/L) of reactants and products.</u> Its value in a chemical reaction depends on the temperature, so it must always be specified.
<u>We will use the the equilibrium constant Kc of the reaction to calculate partial pressure of ethene.</u> The constant Kc for the above reaction is,
Kc =
According to the law of ideal gases,
PV = nRT
where P, V, n and T are the pressure, volume, moles and temperature of the gas in question while R is the gas constant (0.082057 atm L / mol K) .
We can use the ideal gas law to determine the molar concentrations ([x] = n / V) from the gas pressures of ethanol and water, assuming that all gases involved behave as ideal gases. In this way,
PV = nRT → P = (n/V) RT → P = [x] RT → [x] = P / RT
So,
So, the molar concentration of ethene (C₂H₄) will be,
Then, according to the law of ideal gases,
So, when the partial pressure of ethanol is 200 atm and the partial pressure of water is 400 atm, the partial pressure of ethene at 600 K is 2.17x10⁻³ atm.
